Question 1

The pH of a 0.10 M solution of a weak base is 9.82. What is the Kb for this base?

Accepted Answer

A)  6.6 × 10- 4  
B)  2.0 × 10- 5  
C)  2.1 × 10- 4  
D)  4.3 × 10- 8  
E)  8.8 × 10- 8 
A)  6.6 × 10- 4  
B)  2.0 × 10- 5  
C)  2.1 × 10- 4  
D)  4.3 × 10- 8  
E)  8.8 × 10- 8

Question 2

Nitric acid is a strong acid. This means that .

Accepted Answer

A)  HNO3 cannot be neutralized by a weak base 
B)  HNO3 produces a gaseous product when it is neutralized 
C)  HNO3 does not dissociate at all when it is dissolved in water 
D)  aqueous solutions of HNO3 contain equal concentrations of H+(aq) and OH- (aq) 
E)  HNO3 dissociates completely to H+(aq) and NO3- (aq) when it dissolves in water 
A)  HNO3 cannot be neutralized by a weak base 
B)  HNO3 produces a gaseous product when it is neutralized 
C)  HNO3 does not dissociate at all when it is dissolved in water 
D)  aqueous solutions of HNO3 contain equal concentrations of H+(aq) and OH- (aq) 
E)  HNO3 dissociates completely to H+(aq) and NO3- (aq) when it dissolves in water

Question 3

Classify the following compounds as weak acids (W) or strong acids (S):
Hypochlorous acid perchloric acid chloric acid

Accepted Answer

A)  S W W 
B)  S S S 
C)  W W W 
D)  W S S 
E)  W S W 
A)  S W W 
B)  S S S 
C)  W W W 
D)  W S S 
E)  W S W

Question 4

What is the pH of a sodium formate solution prepared by adding 0.680 grams of sodium formate to 100.0 ml of water at 25.0 oC? The Ka at 25.0 oC for formic acid is 1.8 × 10- 4.

Accepted Answer

Question 5

Which of the following aqueous solutions has the highest [OH- ]?

Accepted Answer

A)  a 1 × 10- 4 M solution of HNO3 
B)  pure water 
C)  a solution with a pH of 3.0 
D)  a 1 × 10- 3 M solution of NH4Cl 
E)  a solution with a pOH of 12.0 
A)  a 1 × 10- 4 M solution of HNO3 
B)  pure water 
C)  a solution with a pH of 3.0 
D)  a 1 × 10- 3 M solution of NH4Cl 
E)  a solution with a pOH of 12.0

Question 6

In the reaction
BF3 + F- →BF4-
BF3 acts as a BrØnsted- Lowry acid.

Accepted Answer

A) True 
 B)False

Question 7

Kb for NH3 is 1.8 × 10- 5. What is the pH of a 0.35 M aqueous solution of NH4Cl at 25.0 °C?

Accepted Answer

A)  9.1 
B)  4.3 
C)  11 
D)  9.7 
E)  4.9 
A)  9.1 
B)  4.3 
C)  11 
D)  9.7 
E)  4.9

Question 8

The acid- dissociation constants of phosphoric acid (H3PO4) are Ka1 = 7.5 × 10- 3, Ka2 = 6.2 × 10- 8, and Ka3 = 4.2 × 10- 13 at 25.0 °C. What is the pH of a 2.5 M aqueous solution of phosphoric acid?

Accepted Answer

A)  0.13 
B)  2.5 
C)  0.40 
D)  1.8 
E)  0.87 
A)  0.13 
B)  2.5 
C)  0.40 
D)  1.8 
E)  0.87

Question 9

Of the following acids, is not a strong acid.

Accepted Answer

A)  H2SO4  
B)  HNO2  
C)  HCl 
D)  HClO4  
E)  HNO3 
A)  H2SO4  
B)  HNO2  
C)  HCl 
D)  HClO4  
E)  HNO3

Question 10

What is the conjugate base of OH- ?

Accepted Answer

A)  H2O 
B)  O2-  
C)  O2  
D)  O-  
E)  H3O+ 
A)  H2O 
B)  O2-  
C)  O2  
D)  O-  
E)  H3O+

Question 11

The base- dissociation constant, Kb, for pyridine, C5H5N, is 1.4 × 10- 9. The acid- dissociation constant, Ka, for the pyridinium ion, C5H5NH+, is _ .

Accepted Answer

A)  1.4 × 10- 5 
B)  7.1 × 10- 4 
C)  1.4 × 10- 23 
D)  7.1 × 10- 6 
E)  1.0 × 10- 7 
A)  1.4 × 10- 5 
B)  7.1 × 10- 4 
C)  1.4 × 10- 23 
D)  7.1 × 10- 6 
E)  1.0 × 10- 7

Question 12

The simplest amino acid is glycine.

Accepted Answer

A) True 
 B)False

Question 13

The pH of a 0.15 M aqueous solution of NaZ (the sodium salt of HZ) is 10.7. What is the Ka for HZ?

Accepted Answer

A)  8.9 × 10- 4 
B)  3.3 × 10- 8 
C)  1.3 × 10- 12 
D)  1.6 × 10- 6 
E)  6.0 × 10- 9 
A)  8.9 × 10- 4 
B)  3.3 × 10- 8 
C)  1.3 × 10- 12 
D)  1.6 × 10- 6 
E)  6.0 × 10- 9

Question 14

An aqueous solution at 25.0 °C contains [H+] = 0.0990 M. What is the pH of the solution?

Accepted Answer

A)  1.00 
B)  1.00× 10- 13 
C)  - 1.00 
D)  13.0 
E)  0.0990 
A)  1.00 
B)  1.00× 10- 13 
C)  - 1.00 
D)  13.0 
E)  0.0990

Question 15

In the gas phase reaction below, NH3 is acting as a(n) base but not as a(n) base.

Accepted Answer

A)  Lewis, BrØnsted- Lowry 
B)  Arrhenius, BrØnsted- Lowry 
C)  Arrhenius, Lewis 
D)  BrØnsted- Lowry, Lewis 
E)  Lewis, Arrhenius 
A)  Lewis, BrØnsted- Lowry 
B)  Arrhenius, BrØnsted- Lowry 
C)  Arrhenius, Lewis 
D)  BrØnsted- Lowry, Lewis 
E)  Lewis, Arrhenius

Question 16

The conjugate base of HSO4- is

Accepted Answer

A)  H2SO4  
B)  OH-  
C)  HSO4+  
D)  SO42-  
E)  H3SO4+ 
A)  H2SO4  
B)  OH-  
C)  HSO4+  
D)  SO42-  
E)  H3SO4+

Question 17

The Ka for HCN is 4.9 × 10- 10. What is the value of Kb for CN- ?

Accepted Answer

A)  4.9 × 104 
B)  2.0 × 10- 5 
C)  2.0 × 109 
D)  4.0 × 10- 6 
E)  4.9 × 10- 24 
A)  4.9 × 104 
B)  2.0 × 10- 5 
C)  2.0 × 109 
D)  4.0 × 10- 6 
E)  4.9 × 10- 24

The pH of a 0.10 M solution of a weak base is 9.82. What is the K_bfor this base?

Nitric acid is a strong acid. This means that .

Classify the following compounds as weak acids (W) or strong acids (S): Hypochlorous acid perchloric acid chloric acid

What is the pH of a sodium formate solution prepared by adding 0.680 grams of sodium formate to 100.0 ml of water at 25.0 ^oC? The K_aat 25.0 ^oC for formic acid is 1.8 × 10^-⁴.

Which of the following aqueous solutions has the highest [OH^-]?

In the reaction BF₃+ F^-→BF₄^- BF₃acts as a BrØnsted- Lowry acid.

K_bfor NH₃is 1.8 × 10^-⁵. What is the pH of a 0.35 M aqueous solution of NH₄Cl at 25.0 °C?

The acid- dissociation constants of phosphoric acid (H₃PO₄) are K_a1= 7.5 × 10^-³, K_a2= 6.2 × 10^-⁸, and K_a3= 4.2 × 10^-¹³at 25.0 °C. What is the pH of a 2.5 M aqueous solution of phosphoric acid?

Of the following acids, is not a strong acid.

What is the conjugate base of OH^-?

The base- dissociation constant, K_b, for pyridine, C₅H₅N, is 1.4 × 10^-⁹. The acid- dissociation constant, K_a, for the pyridinium ion, C₅H₅NH⁺, is _ .

The simplest amino acid is glycine.

The pH of a 0.15 M aqueous solution of NaZ (the sodium salt of HZ) is 10.7. What is the K_afor HZ?

An aqueous solution at 25.0 °C contains [H⁺] = 0.0990 M. What is the pH of the solution?

In the gas phase reaction below, NH₃is acting as a(n) base but not as a(n) base.

The conjugate base of HSO₄^-is

The K_afor HCN is 4.9 × 10^-¹⁰. What is the value of K_bfor CN^-?

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Exam 16: Acid-Base Equilibria

The pH of a 0.10 M solution of a weak base is 9.82. What is the Kb for this base?

Nitric acid is a strong acid. This means that .

Classify the following compounds as weak acids (W) or strong acids (S): Hypochlorous acid perchloric acid chloric acid

What is the pH of a sodium formate solution prepared by adding 0.680 grams of sodium formate to 100.0 ml of water at 25.0 oC? The Ka at 25.0 oC for formic acid is 1.8 × 10- 4.

Which of the following aqueous solutions has the highest [OH- ]?

In the reaction BF3 + F- →BF4- BF3 acts as a BrØnsted- Lowry acid.

Kb for NH3 is 1.8 × 10- 5. What is the pH of a 0.35 M aqueous solution of NH4Cl at 25.0 °C?

The acid- dissociation constants of phosphoric acid (H3PO4) are Ka1 = 7.5 × 10- 3, Ka2 = 6.2 × 10- 8, and Ka3 = 4.2 × 10- 13 at 25.0 °C. What is the pH of a 2.5 M aqueous solution of phosphoric acid?

Of the following acids, is not a strong acid.

What is the conjugate base of OH- ?

The base- dissociation constant, Kb, for pyridine, C5H5N, is 1.4 × 10- 9. The acid- dissociation constant, Ka, for the pyridinium ion, C5H5NH+, is _ .

The simplest amino acid is glycine.

The pH of a 0.15 M aqueous solution of NaZ (the sodium salt of HZ) is 10.7. What is the Ka for HZ?

An aqueous solution at 25.0 °C contains [H+] = 0.0990 M. What is the pH of the solution?

In the gas phase reaction below, NH3 is acting as a(n) base but not as a(n) base.

The conjugate base of HSO4- is

The Ka for HCN is 4.9 × 10- 10. What is the value of Kb for CN- ?

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

Aqueous Reactions and Solution Stoichiometry

Electronic Structure of Atoms

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Gases

Intermolecular Forces, Liquids, and Solids

Modern Materials

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Additional Aspects of Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Chemistry of Coordination Compounds

The Chemistry of Life: Organic and Biological Chemistry

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The pH of a 0.10 M solution of a weak base is 9.82. What is the K_bfor this base?

What is the pH of a sodium formate solution prepared by adding 0.680 grams of sodium formate to 100.0 ml of water at 25.0 ^oC? The K_aat 25.0 ^oC for formic acid is 1.8 × 10^-⁴.

Which of the following aqueous solutions has the highest [OH^-]?

In the reaction BF₃+ F^-→BF₄^- BF₃acts as a BrØnsted- Lowry acid.

K_bfor NH₃is 1.8 × 10^-⁵. What is the pH of a 0.35 M aqueous solution of NH₄Cl at 25.0 °C?

The acid- dissociation constants of phosphoric acid (H₃PO₄) are K_a1= 7.5 × 10^-³, K_a2= 6.2 × 10^-⁸, and K_a3= 4.2 × 10^-¹³at 25.0 °C. What is the pH of a 2.5 M aqueous solution of phosphoric acid?

What is the conjugate base of OH^-?

The base- dissociation constant, K_b, for pyridine, C₅H₅N, is 1.4 × 10^-⁹. The acid- dissociation constant, K_a, for the pyridinium ion, C₅H₅NH⁺, is _ .

The pH of a 0.15 M aqueous solution of NaZ (the sodium salt of HZ) is 10.7. What is the K_afor HZ?

An aqueous solution at 25.0 °C contains [H⁺] = 0.0990 M. What is the pH of the solution?

In the gas phase reaction below, NH₃is acting as a(n) base but not as a(n) base.

The conjugate base of HSO₄^-is

The K_afor HCN is 4.9 × 10^-¹⁰. What is the value of K_bfor CN^-?